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BaBr2 + Li2CO3 💧→ BaCO3↓ + 2LiBr

The reaction of barium bromide and lithium carbonate yields barium carbonate and lithium bromide. This reaction is an acid-base reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related categories

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
BaBr2Barium bromide1
Lewis acid
Very soluble in water
Li2CO3Lithium carbonate1
Lewis base
Soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
BaCO3Barium carbonate1
Lewis conjugate
Insoluble in water
LiBrLithium bromide2
Non-redox product

Thermodynamic changes

Changes in standard condition

Reaction of barium bromide and lithium carbonate
ΔrG47.3 kJ/mol
K0.52 × 10−8
pK8.29
BaBr2Crystalline solid + Li2CO3Crystalline solid
💧
BaCO3Crystalline solid + 2LiBrCrystalline solid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1
Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1
Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1
Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
54.547.324
per 1 mol of
54.547.324
per 1 mol of
54.547.324
per 1 mol of
54.547.324
per 1 mol of
27.323.612

Changes in aqueous solution

Reaction of barium bromide and lithium carbonate
ΔrG−31.4 kJ/mol
K3.17 × 105
pK−5.50
BaBr2Ionized aqueous solution + Li2CO3Crystalline solid
💧
BaCO3Crystalline solid + 2LiBrIonized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1
Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1
Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1
Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−19.8−31.438.8
per 1 mol of
−19.8−31.438.8
per 1 mol of
−19.8−31.438.8
per 1 mol of
−19.8−31.438.8
per 1 mol of
−9.90−15.719.4

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1
Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1
Standard
molar entropy
S°
J · K−1 · mol−1
Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
BaBr2 (cr)-757.3[1]-736.8[1]146[1]
BaBr2 (g)-439[1]-473[1]331[1]61.5[1]
BaBr2 (ai)-780.73[1]-768.68[1]174.5[1]
BaBr2 (cr)
1 hydrate
-1068.2[1]
BaBr2 (cr)
2 hydrate
-1366.1[1]-1230.4[1]226[1]
Li2CO3 (cr)-1215.9[1]-1132.06[1]90.37[1]99.12[1]
Li2CO3 (ai)-1234.11[1]-1114.6[1]-29.7[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution

Thermodynamic data of products

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1
Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1
Standard
molar entropy
S°
J · K−1 · mol−1
Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
BaCO3 (cr)-1216.3[1]-1137.6[1]112.1[1]85.35[1]
BaCO3 (ai)-1214.78[1]-1088.59[1]-47.3[1]
LiBr (cr)-351.213[1]-342.00[1]74.27[1]
LiBr (g)224.33[1]33.93[1]
LiBr (ai)-400.041[1]-397.27[1]95.8[1]-73.2[1]
LiBr (cr)
1 hydrate
-662.58[1]-594.29[1]109.6[1]
LiBr (cr)
2 hydrate
-962.7[1]-840.5[1]162.3[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas

References

List of references

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)